Kelvi

Kelvi

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Kelvi

0 pts

The freezing point depression constant (K $_f$ ) of benzene is $5.12$ K kg mol $^{-1}.$ The freezing point depression for the solution of molality $0.078$ m containing a non-electrolyte solute in benzene is (rounded off upto two decimal places):

medium

Solutions

2020

chemistry

$0.80$ K

$0.40$ K

$0.60$ K

$0.20$ K

Explanation

To solve this problem, we will use the formula for freezing point depression: $\\ \Delta T_f = K_f \cdot m \\$ Where: $\\$

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•

\Delta T_f

is the freezing point depression.

\\

•

K_f

is the freezing point depression constant.

\\

•

m

is the molality of the solution.

\\

Given:

\\ K_f = 5.12 \,

K kg mol

^{-1} \\ m = 0.078 \,

mol kg

^{-1} \\

Substitute the given values into the formula:

\\ \Delta T_f = 5.12 \times 0.078 \\

Calculate

\Delta T_f: \\ \Delta T_f = 0.39936 \\

Round off

\Delta T_f

to two decimal places:

\\ \Delta T_f = 0.40 \,

K

\\

Therefore, the freezing point depression for the solution is

0.40 \,

K

. \\

This corresponds to Option 2.